NEETChemistryChemical Bonding and Molecular Structure
Identify the correct increasing order of bond angles in the following species : NO ₂⁺, NO ₃⁻, NO ₂⁻, NH ₄⁺
Options
- ANO ₂⁻ < NH ₄⁺ < NO ₃⁻ < NO ₂⁺
- BNH ₄⁺ < NO ₂⁻ < NO ₃⁻ < NO ₂⁺
- CNH ₄⁺ < NO ₃⁻ < NO ₂⁻ < NO ₂⁺
- DNO ₂⁺ < NO ₃⁻ < NO ₂⁻ < NH ₄⁺
Correct answer
B. NH ₄⁺ < NO ₂⁻ < NO ₃⁻ < NO ₂⁺
Step-by-step solution
According to VSEPR theory and hybridization rules: In NH ₄⁺ , the central nitrogen atom is sp^3 hybridized with zero lone pairs. The geometry is perfectly tetrahedral with a bond angle of 109.5^ . In NO ₂⁻ , the central nitrogen atom is sp^2 hybridized with one lone pair. The ideal angle for sp^2 is 120^ , but due to lone pair-bond pair repulsion, it decreases to approximately 115^ . In NO ₃⁻ , the central nitrogen atom is sp^2 hybridized with zero lone pairs. The geometry is trigonal planar with a bond angle of ex